Conclusion question(s) from a lab we did to find the heat of fusion of ice: Does the value obtained for the molar heat of fusion depend on the volume of water used? Does it depend on the mass of ice
129,123 results
chemistry
1. Given that 50 grams of ice is heated at 20.0 °C to steam at 135.0 °C. i. Show the graph of the changes from ice to steam ii. Calculate the energy needed to change the ice to steam Please use these values: Heat of fusion = 334.16 J g¯1 Heat of

CHEMISTRY
How much heat is needed to melt 150g of ice? and How much heat is needed to change 150g of ice into steam at 110 degrees? My heat of fusion is 361 and my percent error is 8 if you need that. Answers quickly please :(

Chemistry  Heat of Fusion of Ice
Conclusion question(s) from a lab we did to find the heat of fusion of ice: Does the value obtained for the molar heat of fusion depend on the volume of water used? Does it depend on the mass of ice melted? Does it depend on the final temperature of the

physics
A 250g block of ice is removed from the refrigerator at 8.0°C. How much heat does the ice absorb as it warms to room temperature (22°C)? The heat of fusion of water is 3.34105 J/kg.

physics
Years ago, a block of ice with a mass of about 22kg was used daily in a home icebox. The temperature of the ice was 0.0 degrees Celsius when delivered. As it melted, how much heat did a block of ice that size absorb? The latent heat of fusion of water is

physics
How long would it take a 1 200 W heater to melt 1.00 kg of ice at 12.0°C, assuming all the energy from the heater is absorbed by the ice? (Assume the specific heat of the ice is 2 090 J/kg · °C and the latent heat of fusion of water is 3.33 105 J/kg.)

Chemistry
For a chemistry lab, I have to calculate the heat of combustion of paraffin wax. So how would I do that? And for the second part of the lab, I have to calculate the heat of fusion of ice from my data. How would I do that? I'm kind of confused so can I get

Chemistry
Use the heating curve of 50 g of water and the list of values to answer the question. specific heat of ice = 2.10 J/(g·°C) specific heat of water = 4.18 J/(g·°C) specific heat of water vapor = 2.07 J/(g·°C) latent heat of fusion of ice = 333.4 J/g

Chemistry
Topic: Sublimation and Fusion How much heat (in kJ) is required to warm 13.0 g of ice, initially at 14.0 C, to steam at 112.0 °C? The heat capacity of ice is 2.09 J/g⋅°C and that of steam is 2.01 J/g⋅°C. Any help on how to start this is really

Physics
Which provides more cooling for a styrofoam cooler, one with 10 lbs of ice at 0 degrees C or one with 10 lbs of ice water at 0 degrees C. Explain. qice=mass*heat of fusion. qH2O=mass*specific heat x delta T However, you aren't given a two temperatures;

Chemistry
A quantity of ice at 0.0 degrees C was added to 33.6 of water at 21.0 degree C to give water at 0.0 degrees C. How much ice was added? The heat of fusion of water is 6.01 kJ/mol and the specific heat is 4.18 J/(g * degrees C) q = mass x specific heat x

Chemistry
How many kJ of heat are required to convert 1.00 g of ice at 25°C to steam at 125°C? s(ice) = 2.108 J/g·°C s(liquid water) = 4.184 J/g·°C s(steam) = 1.996 J/g·°C heat of fusion = 6.01 kJ/mol heat of vaporization = 40.79 kJ/mol

Physics
How much energy is required to change a 58 g ice cube from ice at −1◦C to steam at 101◦C? The specific heat of ice is 2090 J/kg ·◦ C and of water 4186 J/kg ·◦ C. The latent heat of fusion of water is 3.33 × 105 J/kg, its latent heat of

chemo
How much heat (in kJ) does it take to melt 28.4 grams of ice at 0 °C and raise the temperature of the resulting water to 25 °C? Heat of fusion 334 J/g, Specific heat 4.184 J/g °C ?

Phyics
How much energy is required to change a 57 g ice cube from ice at −4◦C to steam at 107◦C? The specific heat of ice is 2090 J/kg ·◦ C and of water 4186 J/kg ·◦ C. The latent heat of fusion of water is 3.33 × 105 J/kg, its latent heat of

Physics
How much heat must be removed from 456 g of water at 25.0°C to change it into ice at 10.0°C? The specific heat of ice is 2090 J/kg ∙ K, the latent heat of fusion of water is 33.5 × 104 J/kg, and the specific heat of water is 4186 J/kg ∙ K.

Chemistry
How much ice (in grams) be added to lower the temperature of 355 mL of water from 25 ∘C to 5 ∘C ? (Assume the following: the density of water is 1.0 g/mL, the ice is at 0 ∘C, the heat of fusion of ice is 6.02 kJ/mol, and the volume of water produced

PHYSICS HELP PLEASE
How much heat has to be added to change 0.500 kg ice from 10C completely to a steam of 110C. The specific heat of ice, water and steam is 2090 J/kg ⋅K, 4186 J/kg⋅K, 2010 J/kg ⋅K respectively. Given that the heat J/kg, the heat of J/kg. Draw of

Chemistry
Hey, for chemistry class we are given days in the lab to conduct an experiment, then answer a number of questions that correlate with that experiment and how we can make use of it. This week we looked at the Molar Fusion of Ice and there are some questions

Physical Science
A 5.00 kg block of ice at –25 oC is converted to steam at 125 oC. How much energy (in kilojoules) is expended in this process? The following data are provided: a. Specific heat of ice = 2.092 J/g oC b. Latent heat of fusion = 334.72 J/g c. Specific heat

Chemistry
Calculate the heat released when 42.0 g of water at 35.0 degrees Celsius is converted to ice at 5.0 degrees Celsius. The specific heat of ice is 2.03 J/(g C), the molar heat of fusion of ice is 6010 J/mol, and the specific heat of water is 4.18 J/(g C)

Chemistry
Suppose that 100.0 g of ice a 0 degreesC are added to 300.0 g of water at 25.0 degrees . Is this sufficient ice to lower the temperature of water to 5.00 degrees C and still have ice remaining? Calculate the energy (heat) which must be removed from water

Physics
A 35g block of ice at 14°C is dropped into a calorimeter (of negligible heat capacity) containing 400 g of water at 0°C. When the system reaches equilibrium, how much ice is left in the calorimeter? The specific heat of ice is 2090 J(kg K) and the

Chem
A student measures the following data regarding the heat of fusion of ice: 25.8 g ice at 0.0°C is placed into the calorimeter which contains 100.0 g water at 21.7°C. The final temperature comes to 1.5°C. The calorimeter has a heat capacity of 15.6

physics
A 68 g ice cube at −23◦C is dropped into a container of water at 0◦ C. How much water freezes onto the ice? The specific heat of ice is 0.5 cal/g ·◦ C and its heat of fusion of is 80 cal/g. Answer in units of g.

Physics
Ice at 0°C is added to 200gms of water initially at 70°C in a vacuum flask. When 50gms of ice has been added and has all melted the temperature of the flask and the contents become 40°C. When 80gms of ice has been added and has all melted the

PHYSICS
The wattage of a commercial ice maker is 226 W and is the rate at which it does work. The ice maker operates just like a refrigerator and has a coefficient of performance of 3.90. The water going into the unit has a temperature of 15.0°C, and the ice

Chemistry  Melting Ice
The heat of fusion of ice is 6.00 kJ/mol. Find the number of photons of wavelength = 6.78×10^−6 m that must be absorbed to melt 6.80 g of ice.

Chemistry
Heat of Combustion of paraffin wax Initial mass of candle 40.3g Mass of tin calorimeter 41.1g Mass of halffilled calorimeter with water 220.4g Initial temp of water 18.8°C Final temp of water 26.6°C Final mass of candle 38.2g Calculate heat of

math
Problem The latent heat of fusion (solid become liquid) for ice is 79.8 cal/gram. How much ice can we melt with 1000 calories of heat? Problem Which would require more heat, melting 500 g of 0 C ice or turning 500 g of 100 C water into steam? Problem A 500

physics
A 27 g ice cube at −25◦C is dropped into a container of water at 0◦C. How much water freezes onto the ice? The specific heat of ice is 0.5 cal/g · ◦ C and its heat of fusion of is 80 cal/g. Answer in units of g.

Chemistry
Calculate the amount of heat, in kJ, needed to convert 30.0 g of ice at 5.2 oC to liquid water at 58 oC. Specific heat of ice = 2.10 J/(g oC); heat of fusion of ice = 334 J/g; Specific heat of water = 4.18 J/(g oC)

Science
The avg moler heat capacities of ice and water are 37.8 and 75.6jmol1 respectively and the enthalpy of fusion of ice is 6.012kjmol1 the amount of heat required to change 10 gm of ice at 10°c to water at10°c would be

Physics
what mass of ice at 14'c will be needed to cool 200cm3 of an orange drink (essentially water) from 25'c to 10'c! (specific latent heat of fusion of ice =336000) (specific heat capacity of ice = 2100) (specific heat capacity of water = 4200)

physics
How much heat must be removed from 456 g of water at 25.0°C to change it into ice at 10.0°C? The specific heat of ice is 2090 J/kg ∙ K, the latent heat of fusion of water is 33.5 × 104 J/kg, and the specific heat of water is 4186 J/kg ∙ K.

College Chemistry
What is the final temperature, in oC, after a 26.5 g piece of ice, at 0oC, is placed in a styrofoam cup with 122 g of water initially at 73.8oC the specific heat of water = 4.184 JK1g1 The heat of fusion of ice = 333 Jg1

Chemistry
A 13.0g sample of ice at 13.0°C is mixed with 112.0 g of water at 80.0°C. Calculate the final temperature of the mixture assuming no heat loss to the surroundings. The heat capacities of H2O(s) and H2O(l) are 2.08 and 4.18 J/g · °C, respectively, and

physcial science
When 1 kg of ice at 0 degrees Celsius absorbs 80 kilocalories of heat, the ice undergoes a) a change of state b) a loss of energy c) a rise in temperature d) an increase in volulme The heat of fusion of water is 80 kcal/kg. That means that 1 kg of ice will

Chemistry  Heat of Fusion of Ice
I need help with these questions since the lab report needs to be completed like...NOW >_< We were supposed to experimentally determine the heat of fusion of ice and compare it to the accepted value as listed in your reference table.Please help me: Does

chem
The heat of combustion of bituminous coal is 2.50 × 104 J/g. What quantity of the coal is required to produce the energy to convert 137.7 pounds of ice at 0.00°C to steam at 100.°C? specific heat (ice) = 2.10 J/g°C specific heat (water) = 4.18 J/g°C

Chemistry
A quantity of ice at 0.0 degrees C was added to 33.6 of water at 21.0 degree C to give water at 0.0 degrees C. How much ice was added? The heat of fusion of water is 6.01 kJ/mol and the specific heat is 4.18 J/(g * degrees C) q = mass x specific heat x

Science
a 67 gram chunk of ice (Heat of Fusion = 6.0 kJ/mol) in a beaker immersed in a water bath. To produce just enough heat to melt the ice, how many moles of solid NaOH (Heat of Solution = 445.1 kJ/mol) must be added to this system to just melt the ice.

PLZZZ HELP
Heat of Combustion of paraffin wax Initial mass of candle 40.3g Mass of tin calorimeter 41.1g Mass of halffilled calorimeter with water 220.4g Initial temp of water 18.8°C Final temp of water 26.6°C Final mass of candle 38.2g Calculate heat of

Chemistry
Find the amount of heat to be released to convert 40 grams of steam at 108°C to ice at 7°C. The latent heat of fusion and the latent heat of vaporization are 80 cal/g and 540 cal/g respectively. Cp water 4.187 KJ/kg K, Cp ice 2.108 KJ/kg.K, Cp steam

chemistry
What equation will you use to calculate the heat of fusion of ice? The specific heat of water is 4.184 J/(gx°C), and the heat capacity of your calorimeter is 1.0x10^1 J/°C.

physics
. How much thermal energy must be removed from a 0.25kg chunk of ice to lower its temperature by 18C ? The specific heat of ice to is 2100 J/kg ⋅K and the heat of fusion for ice is 334×10^3J/kg.

Jake
If 142.38 g of l water at 21.7 degrees C is placed into a syrofoam cup with 174.36 g of ice at 27.5 degrees C what would be the final temperature of the entire contents at equilibrium? If it is partially frozen, how many g of the ice has melted? given

physics
A 44.0g block of ice at 15.0°C is dropped into a calorimeter (of negligible heat capacity) containing of water at 5.0°C. When equilibrium is reached, how much of the ice will have melted? The specific heat of ice is 2090 J/kg ∙ K, that of water is

chemistry
The heat of fusion of ice is 6.00 kJ/mol. Find the number of photons of wavelength = 6.42 x 10e6 m that must be absorbed to melt 2.00 g of ice.

physics
What is the final equilibrium temperature when 40.0 grams of ice at 0°C is mixed with 5.00 grams of steam at 120°C? The specific heat of ice is 2.10 kJ/kg °C, the heat of fusion for ice at 0°C is 333.7 kJ/kg, the specific heat of water 4.186 kJ/kg °C,

Chemistry
What is the final temperature, in oC, after a 27.0 g piece of ice, at 0oC, is placed in a styrofoam cup with 120 g of water initially at 70.5oC. Assume there is no transfer of heat to or from the surroundings. The specific heat of water = 4.184 JK1g1 The

physics
150g of ice is removed from a freezer at a temperature of 15°C. The ice is left, eventually reaching thermal equilibrium with its surroundings at a temperature of 21°C. If the latent heat of fusion for water is 336 kl/kg, the specific heat capacity of

Chemistry
what is the minimum mass of ice at 0.0C that must be added to 1.00kg of water to cool the water from 25.0C to 12.0C. the heat of fusion is 333J/g; specific heat capacities of ice = 2.06J/gK; the heat capacity of water is 4.184J/gK. I have no clue where to

physics
1) what mass of ice at 14'c will be needed to cool 200cm3 of an orange drink (essentially water) from 25'c to 10'c! (specific latent heat of fusion of ice =336000) (specific heat capacity of ice = 2100) (specific heat capacity of water = 4200)

Chemistry HEAT OF FUSION
What amount of energy is required to melt a 26.9 g piece of ice at 0oC? The heat of fusion of ice = 333 Jg1 Heat required to melt the ice = J What amount of energy must be removed from 120 g of water to cool it from 72.1oC to 12.4oC? Specific heat of

Chemistry
What is the final temperature when 2.50 x 10^5 J are added to 0.950 kg of ice at 0.0 degrees C? The specific heat capacity of water is 4186 J/(kg·degrees C) and the latent heat of fusion for ice is 3.35×10^3 J/kg.

Physics
A 0.0475 kg ice cube at −30.0°C is placed in 0.577 kg of 35.0°C water in a very well insulated container. The latent heat of fusion of water is 334 kJ/kg, the specific heat of ice is 2092 J/(kg · K), and the specific heat of water is 4184 J/(kg · K).

physics
A 1.3 Kg block of ice is initially at a temp of 5 degrees celsius. If 7.5 *10^5 J of heat are added to the ice, what is the final temperature of the system? I multiplied 1.3 Kg of ice by the specific heat of ice (2090), then I divided by the amount of

chem
im working on a lab in chemistry called measuring energy changes :Calorimetry how to you determine the molar latent heat of fusion of ice using q=mcT ?? why was the ice driedbefore it was placed in water? why is hot warer ysed rather than room temp? in

Chemistry(explain Please)
How would i find the following? I just need an explanation. I'm stuck. I have many other questions like this and i need to know how to do them. The specfic heat of ice is 2.05 J/g. In a calorimeter, 10.0 g of ice melts at 0oC. The enthalpy of fusion of the

Will Someone please respond! Chem
How would i find the following? I just need an explanation. I'm stuck. I have many other questions like this and i need to know how to do them. The specfic heat of ice is 2.05 J/g. In a calorimeter, 10.0 g of ice melts at 0oC. The enthalpy of fusion of the

chemistry
how much heat is required to completely vapporize 2.3 grams of ice starting at 50 degrees Celsius? (the specific heat of ice is 2.0 J/g.C; the specific heat of water is 4.184 J/g.C; the heat of fusion is 333 J/g; and the heat of vaporization is 22601 J/g)

i need help physics
. How much thermal energy must be removed from a 0.25kg chunk of ice to lower its temperature by 18C ? The specific heat of ice to is 2100 J/kg ⋅K and the heat of fusion for ice is 334×10^3 J/kg.

chemistry
HELPPPP!!!! This is a lab, and i need help with the equations please!! Thank you !! Heat of fusion data table : Mass of foam cup = 3.57g Mass of foam cup + warm water = 104.58g Mass of foam cup + warm water + melted ice = 129.1g Temperature of warm water =

physics 10
1.) 100 kJ of heat is added to 600g of zinc at 20 C and 75g of it melts. If the specific heat of zinc is 0.385 kJ/kgC and it melts at 420 C. What is its heat of fusion? 2.) If all the heat lost by 1kg of water at 0 C when it turns into ice at 0 C could be

Chemistry
A 63 gram block of an unknown metal at 88 degrees C was dropped into an insulated flask containing approx. 30 g of ice and 30 g of water at 0 degrees C. After the system had reached a steady temp. it was determined that 12.1 g of ice had melted. What is

Enthalpy of a Phase Change
How many grams of ice at 20.1C can be completely converted to liquid at 9.9C if the available heat for this process is 4.58×103 kJ? For ice, use a specific heat of 2.01 J/(g*C) and Heat of Fusion is = 6.01 kJ/mol.

HELPP CHEMM
Heat of fusion of ice lab Initial mass of empty cup calorimeter 9.55g Initial mass of water 200.15g Initial mass of ice + water 209.7g Initial temp of water 41.9°C Initial mass of ice 26.9g Final mass of cup 9.55g Final mass of water 227.05g Final mass of

physics
a 75kg skater is travelling at 15m/s stops suddenly on the ice. If the ice is at 0 degrees and it is assumed that all of the skaters energy is converted to heat, how much ice does he melt? (latent heat of fusion for water is 3.3x10^5 J/kg)

PHYSICS
The wattage of a commercial ice maker is 226 W and is the rate at which it does work. The ice maker operates just like a refrigerator and has a coefficient of performance of 3.90. The water going into the unit has a temperature of 15.0°C, and the ice

physics
The wattage of a commercial ice maker is 226 W and is the rate at which it does work. The ice maker operates just like a refrigerator and has a coefficient of performance of 3.90. The water going into the unit has a temperature of 15.0°C, and the ice

had
A 0.106 kg ice cube is taken out of a freezer with temperature 16°C. It is then added to a glass of water with mass 0.25 kg. The water initially has a temperature of 24.2 °C. Assume no heat is added or lost to the surroundings. Calculate the amount heat

Physics
Find the heat necessary to change 2.5kg of water (ice) at 2 degrees C to steam at 105 degrees C. specific heat ice= 2060 specific heat water= 4180 specific heat steam= 2020 heat of fusion= 3.34X10^5 heat of vaporization= 2.26X10^6

physics
latent heat of fusion of ice is 3.36exp5 j/kg and its specific heat is 1200j/mole.k.. 2kg of ice is at 10degC how much ice will be melt when a heat of 1.42exp5 joule is provided completely? a) 0.5kg b) 1.5kg c) 2kg d) 1kg

Chemistry
I'm sorry But I'm still so badly stuck and I don't get it Initial mass of candle 40.3g Mass of tin calorimeter 41.1g Mass of halffilled calorimeter with water 220.4g Initial temp of water 18.8°C Final temp of water 26.6°C Final mass of candle 38.2g

physics
At a picnic, a Styrofoam cup contains lemonade and ice at 0 degree C. The thickness of the cup is 2.0*10^3m, and the area is 0.016 m^2. The temperature at the outside surface of the cup is 35 degree C. The latent heat of fusion for ice is 3.35*10^5 J/kg.

Chemistry
What amount of energy is required to melt a 27.4 g piece of ice at 0oC? The heat of fusion of ice = 333 Jg1 Heat required to melt the ice 9.12e3 = J What amount of energy must be removed from 123 g of water to cool it from 71.6oC to 9.41oC? Specific heat

PHYSICS
find the heat of fusion of ice M copper calorimeter= 50 g M h20 200 g at 30 C M ice=20.45 at 0 C t2= 20C

physics
7150/(33.5e4) = g ice doesn't work. Am I calculating incorrectly? heat of fusion for water is 334 J/g. You want it in J/g since q is given in the problem in J. The answer will be in units of grams of ice. You will need to change to kg since the problem

Chem
A 135g sample of ice is in a freezer at 21 degrees celsius. It is removed from the freezer and allowed to melt and the resulting water warms up to the room temperature of 23 degrees celsius. How much energy is absorbed by the 135g sample? The specific

Physics
A calorimeter with specific heat of 490x10^2J/kg^1K^1 has a mass of 2.00x10^1kg that contains 3.00x10^1kg of liquid water at 40C. If 5.00x10^2kg of ice at 0C is dropped into the water. Find the final temperature of the mixture where the ice has melted

Science
I'm going crazy! The heat necessary to change the state of water between a solid and a liquid is called the latent heat of vaporization, latent heat of solidification, latent heat of fusion, latent heat of liquefaction, or none of the above. I thought it

science
150g of ice is removed from a freezer at a temperature of 15°C. The ice is left, eventually reaching thermal equilibrium with its surroundings at a temperature of 21°C. If the latent heat of fusion for water is 336 kl/kg, the specific heat capacity of

physics
a) Two 36 g ice cubes are dropped into 300 g of water in a thermally insulated container. If the water is initially at 19°C, and the ice comes directly from a freezer at 19°C, what is the final temperature at thermal equilibrium? (b) What is the final

Physics! HElp
A g ice cube at 15.0oC is placed in g of water at 48.0oC. Find the final temperature of the system when equilibrium is reached. Ignore the heat capacity of the container and assume this is in a calorimeter, i.e. the system is thermally insulated from the

Chemistry
Calculate the energy required to change the temperature of 256.7 mL of water at 22.0 degrees celsius to ice at a temperature of 25.5 degrees celsius. It also tells me to look up the heat of fusion and specific heat. I don't know what I need the heat of

physics
A 37.0 g ice cube at 15.0 degreesC is placed in 224 g of water at 48.0 degreesC. Find the final temperature of the system when equilibrium is reached. Ignore the heat capacity of the container and assume this is in a calorimeter, i.e. the system is

physics
A 37.0 g ice cube at 15.0 degreesC is placed in 224 g of water at 48.0 degreesC. Find the final temperature of the system when equilibrium is reached. Ignore the heat capacity of the container and assume this is in a calorimeter, i.e. the system is

physics
A 37.0 g ice cube at 15.0 degreesC is placed in 224 g of water at 48.0 degreesC. Find the final temperature of the system when equilibrium is reached. Ignore the heat capacity of the container and assume this is in a calorimeter, i.e. the system is

Chemistry HEAT OF FUSION
What is the final temperature, in oC, after a 15.0 g piece of ice, at 0oC, is placed in a styrofoam cup with 128 g of water initially at 74.0oC. Assume there is no transfer of heat to or from the surroundings. The specific heat of water = 4.184 JK1g1 The

physics
An open container holds ice of mass 0.540 kg at a temperature of 18.7 c The mass of the container can be ignored. Heat is supplied to the container at the constant rate of 790 J/minute. The specific heat of ice to is 2100 J/kg . K and the heat of fusion

physic
c. A 2 kg block of ice has been stored in a chiller at a constant 0°C. In order to carry out an investigation, the block of ice needs to be turned into water at a temperature of 75°C. Calculate how much heat energy is required to change the block of ice

Physics
A calorimeter has a mass of 100g and a specific heat of 0.900 cal/g˚c and contains 400g of water at 40˚c. when 91g of ice at 0.0˚c is added and completely melted, the temperature of the water is 18.2˚c. calculate the heat fusion of the ice

Physics
3. A calorimeter has a mass of 100g and a specific heat of 0.900 cal/g˚C and contains 400g of water at 40˚C. When 91g of ice at 0.0˚C is added and completely melted, the temperature of the water is 18.2˚C. Calculate the heat fusion of the ice

Physics
Latent heat question: Your car's windshield is covered with a .58 cm thick layer of ice. The ice has an area of 1.6m^2. If the temperature of the ice is 2C, how much heat is required to melt all the ice?

Chemistry
A 14.0g sample of ice at 18.0°C is mixed with 122.0 g of water at 87.0°C. Calculate the final temperature of the mixture assuming no heat loss to the surroundings. The heat capacities of H2O(s) and H2O(l) are 2.08 and 4.18 J/g · °C, respectively, and

Chemistry
A 19.6 g sample of ice at 10.0°C is mixed with 100.0 g of water at 75.4°C. Calculate the final temperature of the mixture assuming no heat loss to the surroundings. The heat capacities of H2O(s) and H2O(l) are 2.08 and 4.18 J g1 °C1, respectively,

chemistry
A 13.0g sample of ice at 13.0°C is mixed with 105.0 g of water at 78.0°C. Calculate the final temperature of the mixture assuming no heat loss to the surroundings. The heat capacities of H2O(s) and H2O(l) are 2.08 and 4.18 J/g · °C, respectively, and

biology
A 28.0g sample of ice at 18.0°C is mixed with 124.0 g of water at 85.0°C. Calculate the final temperature of the mixture assuming no heat loss to the surroundings. The heat capacities of H2O(s) and H2O(l) are 2.08 and 4.18 J/g · °C, respectively, and

Chemisrty
A 10.0 g sample of ice at 14.0°C is mixed with 124.0 g of water at 81.0°C. Calculate the final temperature of the mixture assuming no heat loss to the surroundings. The heat capacities of H2O(s) and H2O(l) are 2.08 and 4.18 J/g°C, respectively, and the